Chemical Kinetics and Nuclear ChemistryMedium
Question
For an elementary chemical reaction, the Arrhenius plot is given below.
If the energy of activation is $6.64\text{ }kJ{\text{ }mol}^{- 1}$ and $R = 8.3\text{ }J{\text{ }K}^{- 1}{\text{ }mol}^{- 1}$, the temperature at which the rate constant becomes $e^{2}{\text{ }\min}^{- 1}$, is
Options
A.200 K
B.250 K
C.125 K
D.150 K
Solution
Sol. [Key Concept: Arrhenius plot — activation energy and A]
$lnk = lnA - \frac{E_{a}}{RT}$
$$\begin{matrix} & ln\left( e^{2} \right) = 6 - \frac{6.64 \times 10^{3}\text{ }J{\text{ }mol}^{- 1}}{8.3{JK}^{- 1}{\text{ }mol}^{- 1} \times T} \\ & 2 = 6 - \frac{6.64 \times 10^{3}}{8.3 \times T} \\ & \text{ }T = \frac{6.64 \times 10^{3}}{8.3 \times 4} = 200\text{ }K \end{matrix}$$
Create a free account to view solution
View Solution FreeTopic: Chemical Kinetics and Nuclear Chemistry·Practice all Chemical Kinetics and Nuclear Chemistry questions
More Chemical Kinetics and Nuclear Chemistry Questions
Rate of physi-sorption increase with :-...The specific constant of a first order reaction depends on the :...A substance ″A″ decomposes in solution following the first order kinetics. Flask I contains 1 L of 1 M solut...A reaction was found to be second order with respect to the concentration of carbon monoxide. If the concentration of ca...The rate constant for the reaction N2O5 → 4NO2 + O2 is 3.0 × 10−5 s−1. If the rate of reaction is 2.4 × 10−5 mol litre−1...